Chemistry Final Review

Chemistry Final Review - Chemistry Final Review The...

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Unformatted text preview: Chemistry Final Review The following review outline was taken from the notes recorded by a SI (supplemental instruction) student who attended our class. The items listed in this outline are meant as a guide only and are in no way inclusive of all the material that you will be responsible for. These items are also not meant to replaceor minimize the need forthe problems that were assigned at the end of each chapter. Exam Material I. A. Changes 1. Chemical Changes-subatance(s) undergoes reaction to become a new substance(s) 2. Physical Changes-change of state (solid, liquid, gas) B. Properties 1. Intensiveindependent of amount of material present (color, temp, freezing point, density, malleability, etc.) 2. Extensivedependent of amount of material present (mass, volume, surface area) C. Periodic Table 1. Atomic Number 2. Atomic Mass D. Mixtures 1. Heterogeneous-variable composition, can separate out different parts of the mixture (bucket of wood, sand, and rocks) 2. Homogeneous-fixed composition, properties uniform throughout (air, beer, salt water, soda pop, bronze, brass, etc.) I I. A. Law of Definite Proportionsmolecules of a given kind are always made of a certain proportion in a compound. Each compound is made up of a certain number of each king of atom and these atoms are in certain specific proportions based on how many of each there are. B. Law of Multiple Proportionswhen you have two different compounds with the same element and you hold one constant, the other(s) must be in whole number rations to the one held constant C. Periodic Table 1. Rows = periods (period number = shell number) 2. Columns = Groups/families D. Nomenclature of Compounds 1. Binary Compounds: metal first, nonmetal second; IDE ending; eg, NaCl is sodium chloride 2. Molecular Compounds 3. Cation 4. Anion 5. KNOW THE PINK SHEET!!! 6. When making an acid, ate ending changes to ic acid and ite ending changes to ous acid E. Formulas 1. Molecular 2. Empiricalsimplest whole-number ration of the elements in a compound; sometimes is the molecular formula 3. Ionicknow what ions a compound breaks up into I I I. A. Wave nature of light 1. Wavelength 2. Frequencynumber of complete waves per second; units are inverse seconds 3. Speed of light = Frequency x Wavelength. Units of speed are meters per second 4. Energy = Planks constant x Frequency = planks constant x (speed of light / wavelength). Units for energy are joules. 5. Jumping shells: (1 / wavelength) = Ridburgs constant x [ (1 / square of final shell number) - (1 / square of initial shell number) ]; always make answer a positive value. You must remember, however, that jumping to an outer shell requires energy to be put in (energy absorbed); while jumping to an inner energy shell gives off energy....
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This note was uploaded on 04/21/2008 for the course CHEM 1100 taught by Professor Dr.guzinski during the Fall '08 term at Western Michigan.

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Chemistry Final Review - Chemistry Final Review The...

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